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The mole and Avogadro's number

AP.Chem:
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One mole of a substance is equal to 6.022 × 10²³ units of that substance (such as atoms, molecules, or ions). The number 6.022 × 10²³ is known as Avogadro's number or Avogadro's constant. The concept of the mole can be used to convert between mass and number of particles.. Created by Sal Khan.

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  • blobby green style avatar for user allroundphoneix
    what is the relationship between mole and amu?
    1mole of an element is equal to the amu no.of grams but is there another relationship also what is atomic mass and atomic number
    THANK U!
    (130 votes)
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    • blobby green style avatar for user Maree Farquharson
      Hi, this is the way I came to understand the concept of a mole.

      Recall that,
      1 amu = 1.6605 x 10^(-27) kg and
      1 mole = 6.02 x 10^23.

      Therefore,
      1 mole of amus
      = 1 mole of 1.6605 x 10^(-27) kg
      = 6.02x10^23 of 1.6605 x 10^(-27) kg
      = 6.02x10^23 x 1.6605 x 10^(-27) kg ("of" means "x")
      = 0.001kg
      = 1g

      (Please note: Some of the numbers above have been approximated and rounded but for simplicity I've left that stuff out.)

      I think that 1 mole was chosen to be 6.02x10^23 so that when it was multiplied by the amu it would give a nice number like 1g (shown above). I also think they chose to invent the mole because the mass of a proton or neutron is such a small number that they needed a way to descibe the mass in quantities that we can work with.

      I've included an example below showing the same concept to the above example but in a more familiar context. I suggest comparing line-by-line with the above example to see the similarities.

      Example 1: Let's determine the mass of 1 dozen eggs.

      1 egg mass = 60g and
      1 dozen = 12.

      Therefore,
      1 dozen of egg masses
      = 1 dozen of 60g
      = 12 of 60g
      = 12 x 60g
      = 720g

      Example 2: Show that 1 mole of 12C is 12g.

      Recall that,
      1 amu = 1.6605 x 10^(-27) kg and
      1 mole = 6.02 x 10^23.
      12C = 12 amu

      Therefore,
      1 mole of 12C
      = 1 mole of 12 amu
      = 1 mole of 12 x 1.6605 x 10^(-27) kg
      = 6.02x10^23 of 12 x 1.6605 x 10^(-27) kg
      = 6.02x10^23 x 12 x 1.6605 x 10^(-27) kg
      = 0.012 kg
      = 12g

      Generally when working with Avogadro's number and the mass of a proton or neutron, you wouldn't substitute the values in. I was just trying to show why 1 mole of amus equals 1g.

      Anyway, I hope this helps.

      Mars.
      (427 votes)
  • duskpin ultimate style avatar for user Draken
    Is mole a way to express the quantity of a substance?
    (23 votes)
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    • aqualine ultimate style avatar for user nc4228
      Correct. While the mass of 1 mole of a particular substance will vary, 1 mole of ANY substance will ALWAYS have approximately 6.02x10^23 atoms (rounded to 3 significant figures).

      This provides an easy way to express quantities especially when doing multi-step calculations during stoichiometry.
      (23 votes)
  • leaf green style avatar for user Jamin Slack
    So if my understanding of a Mole is correct, basically it is just a tool that was create so that amu could be associated in more simple terms such as a gram?
    (1 vote)
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  • blobby green style avatar for user Gn Chandio
    what was sal telling about relation between 13 almunium and avagadro number when he stooped its making all this confusing?
    (5 votes)
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    • leaf red style avatar for user FTB
      I agree completely with Just Keith's answer of the over complication of this video along with his great detail on the background and mathematics of the mole and atomic mass unit.

      I would just like to add maybe an even more basic explanation that I would employ to start with: when going to the grocery store to shop for you and your family, you would not pick up eggs individually anymore, or say 27 mL of milk or a specific amount of grains of salt (say 5000 grains), you would get say a donzen eggs, a litre/gallon of milk and specific mass/weight in gram/ounce of salt depending upon which unit of measure you use, this being more convenient and manageable number(s) when shopping. The last item, the salt, it would not be feasible to count out grains or even to determine the grain size being consistent, but would be more like the problems encountered for the much smaller atom/compound/molecule.

      Now, for Chemistry when dealing with atoms, compounds or particles of elements, the 'convenient number' is the mole, which makes the use of the atomic mass numbers on the Periodic table manageable and much easier to use both in theoretical calculations and practical experimentation with chemicals. Then I would go into the more specific and accurate details given by Just Keith to explain the concept thoroughly.

      I hope this story/example helps out as a starting point for what can be a very difficult concept depending on how it is approached.
      (14 votes)
  • leaf blue style avatar for user jessica Baccari
    what does amu stand for
    (11 votes)
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  • leaf green style avatar for user somebody
    I was always told that mass, the SI unit for which is the kilogram, was just a measure of how much matter is in an object. However, the mole is basically measuring just that; the amount of amus, or matter in an object. Yet, both the mole and the kilogram are SI units. What is the difference between the two?
    (15 votes)
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    • male robot hal style avatar for user Andrew M
      The mole counts the number of particles, the kilogram (and the amu, too) measures the mass.

      How many eggs are in a dozen? 12. How much mass is there? That's a different question, right?

      How many particles in a mole? 6.02*10^23. What's the mass of those particles? Different question.
      (4 votes)
  • mr pants teal style avatar for user Varun Iyengar
    So, a Mole is just basically a convenient way to convert between grams and atomic mass units?
    (11 votes)
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  • winston baby style avatar for user thakurraghvendra99
    how was the avogadro's number obtained?
    (8 votes)
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    • piceratops ultimate style avatar for user Just Keith
      Avogadro's number is the ratio of the mass of 12 grams of carbon-12 to the mass of 1 atom of carbon-12 measured in grams.

      Or, a little easier to understand, Avogadro's number is the ratio of 1 gram to 1 atomic mass unit but with the atomic mass unit expressed in grams.

      Thus, Avogadro's number has been measured to be 6.022141×10²³.
      (8 votes)
  • blobby green style avatar for user TRILOCHAN BHARDWAJ
    i am confused......
    In the starting of the video it is mentioned that 1 mole is = 1 gram
    but later he said that 1 mole of iron = 56 grams as atomic mass of iron is 56 so why he said that 1 mole is = 1 gram?????
    (0 votes)
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  • marcimus pink style avatar for user Adrija Roy
    I don't quite get it. Does this mean:
    12-gram C-12=1 mole
    16-gram O-16=1 mole
    1-gram H-1=1 mole
    and so on?
    (4 votes)
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Video transcript

- [Instructor] In a previous video, we introduced ourselves to the idea of average atomic mass, which we began to realize could be a very useful way of thinking about a mass at an atomic level, or at a molecular level. But, what we're gonna do in this video is connect it to the masses that we might actually see in a chemistry lab. You're very unlikely to just be dealing with one atom, or just a few atoms, or just a few molecules. You're more likely to deal with several grams of an actual substance. So, how do we go from the masses at an atomic scale to the masses, masses of samples that you see in an actual chemistry lab, or in, I guess you could say, r-scale of the world. Well, the chemistry community has come up with a useful tool. They said, all right, let's think about a given element. So, say, lithium. We know its average atomic mass is 6.94, 6.94 unified atomic mass units per atom, atom of lithium. What if there were a certain number of atoms of lithium such that if I have that number, so times certain, certain number of atoms, then I will actually end up with 6.94 grams, grams of lithium. And, this number of atoms is 6.02214076 times 10 to the 23rd power. So, if you have a sample with this number of lithium atoms, that sample is going to have a mass of 6.94 grams. Whatever its average atomic mass is in terms of unified atomic mass units, if you have that number of the atom, you will have a mass of that same number in terms of grams. Now, you might be saying, is there a name for this number, and there is indeed a name, and it is called Avogadro's number, named in honor of the early 19th century Italian chemist, Amedeo Avogadro. And, in most contexts, because you're not normally dealing with data with this many significant digits, we will usually approximate it as 6.022 times 10 to the 23rd power. Now, there's another word that it's very useful to familiarize yourself with in chemistry, and that's the idea of a mole. Now, what is a mole? It is not a little mark on your cheek. It is not a burrowing animal. Actually, it is both of those things, but, in a chemistry context, a mole is just saying you have this much of something. The word mole was first used by the German chemist Wilhelm Ostwald at the end of the 19th century, and he came up with the word because of its relation to molecule. Now, what does that mean? Well, think about the word dozen. If I say I've got a dozen of eggs, how many eggs do I have? Well, if I have a dozen of eggs, that means I have 12 eggs. So, if I say I have a mole of lithium atoms, how many lithium atoms do I have? That means that I have 6.02214076 times 10 the to 23rd lithium atoms. Exact same idea, it's just that Avogadro's number is much hairier of a number than a dozen. So, let's use our new found powers of the mole and Avogadro's number to start doing some useful things. Let's say that someone were to walk up to you and say, hey, you, I have a 15.4 milligram sample of germanium. How many atoms of germanium am I dealing with? Pause this video and try to think about that. So, let me clear out some space the periodic table of elements was taking up. All right, so we started off with 15.4 milligrams of germanium. The first step might be hey, let's convert this to grams of germanium. And so, we can do a little bit of dimensional analysis. We can just multiply this, for every one gram of germanium that is equivalent to 1,000 milligrams, milligrams of germanium. And so, if you essentially multiply by one thousandth or divide by 1,000, we're gonna get the grams of germanium. And, you can see that in the dimensional analysis by seeing that that is going to cancel out with that leaving us with just the grams of germanium. And, now that we have an expression for grams of germanium, we can think about moles of germanium. So, how do we do that? Well, we're going to multiply by some quantity, and in the denominator we're going to want grams of germanium for the dimensional analysis to work out, grams of germanium, and in the numerator we want the new expression to be in terms of moles of germanium. So, one mole of germanium is equal to how many grams of germanium? Well, we see it right over here. Germanium's molar mass is 72.63 grams per mole. So, for every mole, we have 72.63 grams of germanium. And, you can see that the units work out. These grams of germanium are going to cancel with the grams of germanium just leaving us with moles of germanium. In an actual chemistry practice, finding out the moles of a substance might actually be the most useful thing, but if you wanted to find out the actual atoms of germanium that we're dealing with, we will just multiply by the number of atoms you have per mole. And, this is going to be true for any element. For every mole, you have Avogadro's number of atoms. And, we're going to approximate that as 6.022 times 10 to the 23rd atoms, atoms of germanium, for every one mole, mole of germanium. And so, just to review what we just did, we had milligrams of germanium. You multiply these two together, you'll have grams of germanium, which makes sense, you're essentially just dividing by 1,000. If you were to multiply your grams of germanium times the moles per gram, which is really just the reciprocal of this molar mass we got here, and just to make sure where it makes sense, the units work out nice with the dimensional analysis, this right over here tells you your moles, moles of germanium. And then, if you take your moles and then you multiply it by Avogadro's number, it tells you how many atoms of germanium we have, and that makes sense. If I told you I had a certain number of dozen of eggs, if I wanted to know how many eggs that is I would multiply by 12. So, this whole expression is the number of atoms, atoms of germanium. So, we have 15.4 milligrams. If we wanna figure out how many grams we have, we then divide by 1,000, that's what our dimensional analysis tells us, and it also makes logical sense, divided by 1,000. So, this is how many grams we have. And then, if we wanna figure out how many moles, and it's going to be a small fraction of a mole because a mole is 72.63 grams per mole, we have a small fraction of a gram, much less 72.63 grams. And so, we saw from our analysis to figure out the number of moles, we're now going to essentially divide by 72.63, so divided by 72.63 is equal to, this is the number of moles of germanium we have. And, if we wanna figure out the number of atoms of germanium, we'll then multiply that times Avogadro's number. So, times 6.022 times 10 to the 23rd, and this EE button means times-10-to-the, EE 23rd power, so that's how you do it on a calculator. And then, that gives us this many atoms. And, let's see, just to get our significant digits here, our significant figures, out of all of the things we multiplied, see we had four significant digits here, four significant digits here, but we only had three over here, so I'm going to round to three significant digits. So, I'll go to 1.28 times 10 to the 20th atoms. So, we have approximately 1.28 times 10 to the 20th atoms of germanium, which is a lot.